1.5 - Ideal Gases
No description yet. This curated deck is ready for daily study.
Card preview (19)
if the amount, temperature and pressure is the same, how much volume will an ideal gas take up compared to another ideal gas?
the same
How can we calculate number of moles in an ideal gas?
n=Volume of sample/volume per mole
What does Boyle’s law relate?
pressure and volume
What must be constant for the use of Boyle’s Law?
temperature and moles
What is the equation for boyle’s law?
P1xV1 = P2xV2
What does Charles’ law relate?
temperature and volume
What must be constant for charles’ law to be used.
pressure and moles
What is the equation for charles’ law?
V1/T1 = V2/T2
What does Gay-Lussac’s law relate?
pressure and temperature
what must be constant to use gay-lussac’s law?
volume and moles
what is the equation for gay lussac’s law?
T1/P1 = T2/P2
What does the combined gas law relate?
volume, temperature and pressure
What must be constant to use the combined gas law?
moles
What is the formula for the ideal gas law?
PV = nRT
How does the ideal gas law differ from the other gas laws?
it does not have changing volumes, temperatures, or pressures
What does deviation from an ideal gas depend on?
what gas it is, and perameters like pressure and temperature
when do the greatest deviations from ideal gas behavior occur?
at extreme low temperature and extreme high pressure
Why do the greatest deviations from ideal gas behavior occur at extreme high pressures?
because particles are close together and feel more intermolecular forces (attraction between particles), there is less volume per gas particle
Why do the greatest deviations from ideal gas behavior occur at extreme low temperatures?
because kinetic energy also drops which means less random motion, larger intermolecular forces and harder to maintain a gaseous state